Which element is reduced in the reaction below? I2 + MnO2 + H2O ? I- + MnO4- + H+
I2 + MnO2 + H2O ? I- + MnO4- + H+
Mn oxidation number increases from + 4 to +7. So it is oxidized.
Iodine oxidation number decreases from 0 to -1. So iodine is reduced.
I is reduced>>>>answer
Which element is reduced in the reaction below? I2 + MnO2 + H2O ? I- +...
What is this balanced equation?
MnO4−(aq) +
I−(aq) I2(s) +
MnO2(s)
I got 2MnO4-(aq) +
6I-(aq) +
4H2O(l) ⇌ 3I2(s)
+ 2MnO2(s) + 8OH-(aq)
but webassign is saying it's wrong.
edit: nevermind, figured it out. 2
MnO4-(aq) + 8
H+(aq) +
6I-(aq) ⇌ 3
I2(s) + 2 MnO2(s) + 4
H2O(l)
Calculate values for the following cells. Which reactions are spontaneous as written (under standard conditions)? Balance the equations. Standard reduction potentials are found in the Standard Reduction Potentials table. (Use the lowest possible whole...
Consider the chemical reaction below, KMnO4 + Na2SO3 + H2O → MnO2 + Na2SO4 + KOH Determine if each of the following statement is True or False. 1. The oxidation state of Mn in MnO2 is +2. 2. The oxidation state of S in Na2SO3 is the same as that in Na2SO4. 3. MnO4− gains electrons to form MnO23. 4. Na2SO3 is the oxidizing agent.
118 HNO: Mn + H2O + NO MnO2 + H + Oxidation Half Reaction: Reduction Half Reaction: Oxidizing agent: Reducing agent 4. PbO2 + Mn?' + SO42- + H P bSO4 + MnO4 + H2O Oxidation Half Reaction: Reduction Half Reaction: Oxidizing agent: Reducing agent 5._HNO: + Cr2O72- + H → Cr + NO + H2O Oxidation Half Reaction: Reduction Half Reaction: Oxidizing agent: Reducing agent 6. Mn?+ CIO, MnO2 + CIO Oxidation Half Reaction: Reduction Half Reaction: Oxidizing agent:...
Balance the following REDOX reaction in basic solution: I2(s) + MnO2(s) ---> I-(aq) + MnO4-(aq) (E0 = -0.060 V) The equilibrium constant for this reaction at 25 degrees C is: 8.30 X 10-7 b. 1.38 X 10-7 c. 0.36 d. 8.30 X 107
In a particular redox reaction, MnO2 is oxidized to MnO4- and Ag+ is reduced to Ag. Complete and balance the equation for this reaction in acidic solution. Phases are optional._______ _______
Balance the following redox reactions: Fe^2+ + MnO4^- + H^+ → Fe^3+ + Mn^2+ + H2O Mn^2+ + MnO4^- + …→ MnO2 + … IO3^- + I^- + H^+ → I2 + H2O
In the following balanced reaction equation, identify which element is being reduced, which element is being oxidised and how many electrons are being transferred in the reaction. 3CH3CH2OH + 2Cr2O7 2− + 16H+ ⇌ 3CH3COOH + 4Cr3+ + 11 H2O (A) Cr reduced, C oxidised, 4 e− transferred (B) C reduced, H oxidised, 3 e− transferred (C) Cr reduced, H oxidised, 4 e− transferred (D) Cr reduced, C oxidised, 12 e− transferred (E) C reduced, Cr oxidised, 16 e− transferred
For each of the following redox reactions, determine which element is being reduced and which is being oxidized. (help it should be a one element answer!!) (a) MnO2(aq) + K2C2O4(aq) + 2 H2SO4(aq) → MnSO4(aq) + K2SO4(aq) + 2 CO2(g) + 2 H2O(l) element being reduced : Mn Correct: Your answer is correct. element being oxidized: ?? (c) 2 CrO3(aq) + 3 CH3CH2OH(aq) → Cr2O3(aq) + 3 CH3CHO(aq) + 3 H2O(l) element being reduced ?? element being oxidized ??
What element is being reduced in the following redox reaction? C3H8O2(aq) + KMnO4(aq) → C3H2O4K2(aq) + MnO2(aq) A.C B.K C.H D.O E.Mn
Which element is reduced in the reachen below? I t Mo Oy + H+ Iz + M nO + H₂O D) Mn.